The ionisation potential of hydrogen atom is -13.6 eV. An electron in the ground state of a hydrogen atoms absorbs a photon of energy 12.75 eV. How many different spectral line can one expect when the electron make a downward transition?

Question

The ionisation potential of hydrogen atom is -13.6 eV. An electron in the ground state of a hydrogen atoms absorbs a photon of energy 12.75 eV. How many different spectral line can one expect when the electron make a downward transition? (A) 1 (B) 4 (C) 2 (D) 6

Tardigrade Admin · Accepted Answer

E=E1 / n2 Energy used for excitation is 12.75 eV i e,(-13.6+12.75) eV =-0.85 eV <img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/physics/ad53908b301f63e425ffed7eb0f11086-.png" /> Energy levels of H-atom The photons of energy 12.75 eV can excite the fourth level of H-atom. Therefore, six lines will be emitted, (n ((n-1)/2). lines )

Q. The ionisation potential of hydrogen atom is $- 13.6 e V$ . An electron in the ground state of a hydrogen atoms absorbs a photon of energy $12.75 e V$ . How many different spectral line can one expect when the electron make a downward transition?

1

4

2

6

$E = E_{1} / n^{2}$
Energy used for excitation is $12.75 e V$
$i e, (- 13.6 + 12.75) e V = - 0.85 e V$

Energy levels of H-atom
The photons of energy $12.75 e V$ can excite the
fourth level of $H$ -atom. Therefore, six lines will be emitted, $(n \frac{( n - 1 )}{2}$ lines $)$

Q. The ionisation potential of hydrogen atom is −13.6eV. An electron in the ground state of a hydrogen atoms absorbs a photon of energy 12.75eV. How many different spectral line can one expect when the electron make a downward transition?

1

4

2

6

E=E1​/n2 Energy used for excitation is 12.75eV ie,(−13.6+12.75)eV=−0.85eV Energy levels of H-atom The photons of energy 12.75eV can excite the fourth level of H-atom. Therefore, six lines will be emitted, (n2(n−1)​ lines )

Q. The ionisation potential of hydrogen atom is $- 13.6 e V$ . An electron in the ground state of a hydrogen atoms absorbs a photon of energy $12.75 e V$ . How many different spectral line can one expect when the electron make a downward transition?

$E = E_{1} / n^{2}$
Energy used for excitation is $12.75 e V$
$i e, (- 13.6 + 12.75) e V = - 0.85 e V$

Energy levels of H-atom
The photons of energy $12.75 e V$ can excite the
fourth level of $H$ -atom. Therefore, six lines will be emitted, $(n \frac{( n - 1 )}{2}$ lines $)$